Based on these descriptions, write a balanced equation and the corresponding
-
a. Carbonyl fluoride.
b. Copper metal displaces sliver(l) eon from aqueous solution, producing slyer metal and an aqueous solution of copper(ll) ion.
c. Peroxodisulfate ion,
(a)
Interpretation:
The balanced chemical equation and the Kc expression for the following reversible reaction should be determined:
Carbonyl fluoride, COF2(g), decomposes into gaseous carbon dioxide and carbon tetrafluoride.
Concept introduction:
The balanced reaction is that chemical reaction in which the number of atoms of each element in the product side and on reactant side are equal.
The relationship between the concentration of products and reactants at equilibrium for a general reaction:
Where A, B, C, and D represents chemical species and a, b, c, and d are the coefficients for balanced reaction.
The equilibrium expression, Kc for reversible reaction is determined by multiplying the concentrations of products together and divided by the concentrations of the reactants. Each concentration is raised to the power that is equal to the coefficient in the balanced reaction. So, the expression is:
Square brackets represent the concentration.
Answer to Problem 1E
The balanced chemical equation is:
The expression for the equilibrium constant is:
Explanation of Solution
The reversible reaction for the decomposition of carbonyl fluoride, COF2(g), into gaseous carbon dioxide, CO2(g) and carbon tetrafluoride, CF4(g) is:
This reaction is not balanced as:
The number of atoms of C on reactant side is 1 and on product side is 2, the number of atoms of F on reactant side is 2 and on product side is 4 and the number of atoms of O on reactant side is 1 and on product side is 2.
In order to balance the reaction, the coefficient 2 is put before COF2 on the reactant side.
Thus, the balanced chemical equation is:
In the balanced reversible equation, all the species that is reactant and product are in gaseous phase so, the expression for the equilibrium constant is:
(b)
Interpretation:
The balanced chemical equation and the Kc expression for the following reversible reaction should be determined:
Copper metal displaces silver(I) ion from aqueous solution, producing silver metal and an aqueous solution of copper(II) ion.
Concept introduction:
The balanced reaction is that chemical reaction in which the number of atoms of each element in the product side and on reactant side are equal.
The relationship between the concentration of products and reactants at equilibrium for a general reaction:
Where A, B, C, and D represents chemical species and a, b, c, and d are the coefficients for balanced reaction.
The equilibrium expression, Kc for reversible reaction is determined by multiplying the concentrations of products together and divided by the concentrations of the reactants. Each concentration is raised to the power that is equal to the coefficient in the balanced reaction. So, the expression is:
Square brackets represent the concentration.
Answer to Problem 1E
The balanced chemical equation is:
The expression for the equilibrium constant is:
Explanation of Solution
The reversible reaction for the displacement of silver(I) ion, Ag+(aq), in aqueous solution by copper metal, Cu(s) to produce silver metal, Ag (s) and an aqueous solution of copper (II) ion, Cu2+ is:
This reaction is not balanced as:
The charges on both the sides of the reaction is not balanced so in order to balance the reaction, the coefficient 2 is put before Ag+, the reaction becomes:
In order to balance the Ag atoms, the coefficient 2 is put before Ag on the product side.
Thus, the balanced chemical equation is:
In the balanced reaction, the concentrations of pure solids are constant that is they do not change. Thus, they are not included in the equilibrium expression.
(c)
Interpretation:
The balanced chemical equation and the Kc expression for the following reversible reaction should be determined:
Peroxodisulfate ion, S2O82-, oxidizes iron (II) to iron (III) ion in aqueous solution and is itself reduced to sulfate ion.
Concept introduction:
The balanced reaction is that chemical reaction in which the number of atoms of each element in the product side and on reactant side are equal.
The relationship between the concentration of products and reactants at equilibrium for a general reaction:
Where A, B, C, and D represents chemical species and a, b, c, and d are the coefficients for balanced reaction.
The equilibrium expression, Kc for reversible reaction is determined by multiplying the concentrations of products together and divided by the concentrations of the reactants. Each concentration is raised to the power that is equal to the coefficient in the balanced reaction. So, the expression is:
Square brackets represent the concentration.
Answer to Problem 1E
The balanced chemical equation is:
The expression for the equilibrium constant is:
Explanation of Solution
The oxidation of iron (II) ion, Fe2+ to iron (III) ion, Fe3+ by peroxodisulfate ion, S2O82- and gets reduced itself to sulfate ion, SO42- in aqueous solution is:
This reaction is not balanced as:
The number of atoms of S on reactant side is 2 and on product side is 1 and the number of atoms of O on reactant side is 8 and on product side is 4.
In order to balance the charge and atoms in the reaction, the coefficient 2 is put before Fe2+ on the reactant side and coefficient 2 is put before the SO42- and Fe3+ on the product side.
Thus, the balanced chemical equation is:
In the balanced reversible equation, all the species that is reactant and product are in gaseous phase so, the expression for the equilibrium constant is:
Want to see more full solutions like this?
Chapter 15 Solutions
General Chemistry: Principles and Modern Applications (11th Edition)
Additional Science Textbook Solutions
General, Organic, and Biological Chemistry (3rd Edition)
Introductory Chemistry (5th Edition) (Standalone Book)
General Chemistry: Atoms First
Chemistry: The Molecular Nature of Matter
The Organic Chem Lab Survival Manual: A Student's Guide to Techniques
Chemistry: Structure and Properties
- What is the law of mass action? Is it true that the value of K depends on the amounts of reactants and products mixed together initially? Explain. Is it true that reactions with large equilibrium constant values are very fast? Explain. There is only one value of the equilibrium constant for a particular system at a particular temperature, but there is an infinite number of equilibrium positions. Explain.arrow_forwardHydrogen and carbon dioxide react at a high temperature to give water and carbon monoxide. H2(g) + CO2(g) H2O(g) + CO(g) (a) Laboratory measurements at 986 C show that there are 0.11 mol each of CO and H2O vapor and 0.087 mol each of H2 and CO2 at equilibrium in a 50.0-L container. Calculate the equilibrium constant for the reaction at 986 C. (b) Suppose 0.010 mol each of H2 and CO2 are placed in a 200.0-L container. When equilibrium is achieved at 986 C, what amounts of CO(g) and H2O(g), in moles, would be present? [Use the value of Kc from part (a).]arrow_forwardAt room temperature, the equilibrium constant Kc for the reaction 2 NO(g) ⇌ N2(g) + O2(g) is 1.4 × 1030. Is this reaction product-favored or reactant-favored? Explain your answer. In the atmosphere at room temperature the concentration of N2 is 0.33 mol/L, and the concentration of O2 is about 25% of that value. Calculate the equilibrium concentration of NO in the atmosphere produced by the reaction of N2 and O2. How does this affect your answer to Question 11?arrow_forward
- Consider 0.200 mol phosphorus pentachloride sealed in a 2.0-L container at 620 K. The equilibrium constant, Kc, is 0.60 for PCl5(g) PCl3(g) + Cl2(g) Calculate the concentrations of all species after equilibrium has been reached.arrow_forwardBecause carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?arrow_forwardBecause calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?arrow_forward
- For which reactions in Exercise 33 is Kp equal to Karrow_forwardDecomposition of ammonium dichromate is shown in the designated series of photos. In a closed container this process reaches an equilibrium state. Write a balanced chemical equation for the equilibrium reaction. How is the equilibrium affected if more ammonium dichromate is added to the equilibrium system? more water vapor is added? more chromium(III) oxide is added? Decomposition of ammonium dichromate, for Question 4. Decomposition of (NH4)2Cr2O7. Orange, solid (NH4)2Cr2O7 (a) can be ignited by lighting a wick (b), which initiates decomposition (c) forming Cr2O3, the dark green solid in part (d), N2 gas, and water vapor. Energy is transferred to the surroundings by the process.arrow_forwardWrite equilibrium constant expressions for the following reactions. For gases, use either pressures or concentrations. (a) 2 H2O2(g) 2 H2O(g) + O2(g) (b) CO(g) + O2g CO2(g) (c) C(s) + CO2(g) 2 CO(g) (d) NiO(s) + CO(g) Ni(s) + CO2(g)arrow_forward
- An equilibrium involving the carbonate and bicarbonate ions exists in natural waters: HCO5_(aq) «=* H+(aq) + COf-(aq) Assuming that the reactions in both directions are elementary' processes: Write rate expressions for the forward and reverse reactions. Write an expression for the equilibrium constant based on the rates of the forward and reverse reactions.arrow_forwardConsider the system 4NH3(g)+3O2(g)2N2(g)+6H2O(l)H=1530.4kJ (a) How will the concentration of ammonia at equilibrium be affected by (1) removing O2(g)? (2) adding N2(g)? (3) adding water? (4) expanding the container? (5) increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?arrow_forwardA 0.72-m01 sample of PCl5 is put into a 1.00-L vessel and heated. At equilibrium, the vessel contains 0.40 mol of PCl3(g ) and 0.40 mol of Cl2(g). Calculate the value of the equilibrium constant for the decomposition of PCl5 to PCl3 and Cl2 at this temperature.arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning